CHEM 107: General Chemistry I – Course Syllabus and Study Guide Overview

Course Description and Structure

General Chemistry I is the foundational course in a two-semester sequence designed to introduce students to the core principles of chemistry. The course emphasizes a qualitative, 'big picture' understanding of chemical concepts, bridging the gap between physics and biology. It combines lectures, laboratory work, and active learning strategies to foster deep comprehension and practical skills.

• Lecture: 3 sessions per week (50 minutes each), focusing on problem-solving and discussion.

• Laboratory: 3 hours per week, emphasizing hands-on experimentation and data recording.

• Pre-class Preparation: Students are expected to watch pre-recorded lecture videos and complete textbook readings before class.

• Active Engagement: In-class time is dedicated to addressing questions and collaborative problem-solving.

Learning Outcomes

Upon successful completion of CHEM 107, students will be able to:

• Perform unit conversions with correct use of significant figures and scientific notation.

• Apply atomic theory and periodic trends to predict and discuss elemental properties.

• Distinguish between substances and mixtures, and between chemical and physical changes.

• Name ionic and molecular compounds from formulas and vice versa.

• Balance chemical equations and use the mole concept for stoichiometric calculations.

• Apply thermochemical concepts to chemical reactions.

• Use gas laws to solve problems involving gases.

• Draw and interpret Lewis structures.

• Utilize quantum mechanical concepts to understand chemical bonding.

• Demonstrate accurate laboratory measurement and data recording skills.

Key Topics Covered (Correspondence to General Chemistry Chapters)

• Matter, Measurement & Problem Solving (Ch.1)

• Atoms & Elements (Ch.2)

• Molecules and Compounds (Ch.3)

• Chemical Reactions and Quantities (Ch.4)

• Thermochemistry (Ch.7)

• Gases (Ch.6)

• Chemical Bonding and Quantum Mechanics (Ch.8, Ch.10)

• Lab Techniques and Procedures (BONUS)

• Mathematical Operations in Chemistry (Appendix I)

Assessment and Grading Structure

Student performance is evaluated through a combination of quizzes, homework, exams, laboratory work, and a comprehensive final exam. The grading breakdown is as follows:

Note: No extra credit is available. Students must pass both lecture and lab components to pass the course.

Letter Grade Ranges

Course Policies and Expectations

• Attendance: Regular attendance is required. Excessive absences may result in referral or withdrawal.

• Pre-lecture Quizzes: Random, unannounced quizzes based on lecture videos; lowest two scores dropped.

• Homework: Weekly assignments (online and written); two 24-hour extensions allowed per semester.

• Exams: Four in-class exams (lowest dropped); make-up exams only for approved absences.

• Final Exam: Comprehensive; scheduled by Registrar.

• Lab: Must pass both lecture and lab to pass the course.

• Academic Integrity: Strict adherence to college policies; all incidents reported to the Dean.

• AI Policy: Use of AI tools (e.g., ChatGPT) is prohibited on assignments unless explicitly allowed.

Support and Resources

• Instructor: Dr. Dan Griffith (office hours and appointments available).

• Supplemental Instruction (SI): Peer-led sessions and tutoring available for both sections.

• Textbook: Chemistry: A Molecular Approach, 6th ed., Tro (Pearson, 2024).

• Online Homework: Mastering Chemistry platform.

• Additional Resources: Moodle course site, centralized student support site.

Diversity and Inclusion Statement

The Chemistry Department values diversity and strives for an inclusive, respectful environment. All students are expected to contribute to a culture free from discrimination and harassment.

Key Skills and Concepts for Success

• Unit Conversions: Mastery of converting between units using dimensional analysis.

• Significant Figures: Proper application in calculations and reporting results.

• Atomic Structure: Understanding protons, neutrons, electrons, and isotopes.

• Periodic Table: Recognizing trends (atomic radius, ionization energy, etc.).

• Chemical Nomenclature: Naming and writing formulas for compounds.

• Stoichiometry: Using the mole concept and balanced equations to relate quantities.

• Thermochemistry: Calculating energy changes in chemical reactions.

• Gas Laws: Applying relationships such as Boyle's, Charles's, and the Ideal Gas Law.

• Lewis Structures: Drawing and interpreting electron dot diagrams.

• Quantum Mechanics: Basic principles underlying chemical bonding.

• Laboratory Skills: Accurate measurement, data recording, and safety.

Example: Dimensional Analysis for Unit Conversion

To convert 25.0 grams of water to moles:

• Molar mass of water (H2O): 18.02 g/mol

• Calculation:

Example: Balancing a Chemical Equation

Balance the reaction of hydrogen and oxygen to form water:

Additional info:

• This syllabus overview is based on the provided course document and standard General Chemistry I content.

• For detailed chapter-by-chapter study notes, refer to the course textbook and lecture materials.